Answer:
Yes
Explanation:
Sergei's question is a scientific question because it's based on observations and could be answered through an investigation. His question has a narrow focus, addresses a gap in his knowledge, and may lead to a hypothesis that can be tested.
Umm where are the choises
Answer:
Increasing temperature
Explanation:

Enthalpy of the reaction = -393.5 kJ/mol
Negative sign implies that reaction is exothermic.
Effect of change in reaction condition is explained by Le chateliers principle.
According to Le chateliers principle, if the reaction conditions of a reversible reaction in a state of dynamic equilibirum is changed, the reaction will move in a direction to counteract the change.
1. Increasing the temperature
Forward reaction is exothermic that means temperature increases in forward direction. Backward reaction will be endothermic and so there is decrease in temperature in backward direction or in left direction.
On increasing temperature, reaction will be move in direction to counteract the increased temperature, therefore reaction will move in left direction.
2. Adding O2
If O2 is added, then reaction will move in a direction in which its get consumed. So, reaction will move in forward direction or in right direction.
3. Removing C (s)
Le Chatelier's principle does not apply on solids, so removal of C(s) does not affect the equilibrium.
Logging her results of change day-by-day in a scientific journal. As well as provide as much evidence as possible to support her claim.
The question is incomplete, the complete question is:
Write the net ionic equation for the below chemical reaction:
(c): 
<u>Answer:</u> The net ionic equation is 
<u>Explanation:</u>
Net ionic equation is defined as the equations in which spectator ions are not included.
Spectator ions are the ones that are present equally on the reactant and product sides. They do not participate in the reaction.
(c):
The balanced molecular equation is:

The complete ionic equation follows:

As ammonium and chloride ions are present on both sides of the reaction. Thus, they are considered spectator ions.
The net ionic equation follows:
